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Rashid [163]
3 years ago
14

Determine the volume, in liters, occupied by 0.015 molecules of oxygen at STp?

Chemistry
1 answer:
Arlecino [84]3 years ago
5 0

5.58 X 10^{-25} Litres is the volume, in liters, occupied by 0.015 molecules of oxygen at STP.

Explanation:

Data given:

molecules of oxygen = 0.015

number of moles of oxygen =?

temperature at STP = 273  K

Pressure at STP = 1 atm

volume = ?

R (gas constant) = 0.08201 L atm/mole K

to convert molecules to moles,

number of moles = \frac{molecules}{Avagadro's number}

number of moles = 2.49 x 10^{-26}

Applying the ideal gas law since the oxygen is at STP,

PV = nRT

rearranging the equation:

V = \frac{nRT}{P}

putting the values in the rearranged equation:

V = \frac{2.49 X10^{-26}   X 0.08201 X 273}{1}

V = 5.58 X 10^{-25} Litres.

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The solution is as follows:

K = [Partial pressure of isoborneol]/[Partial pressure of borneol] = 0.106

The molar mass of isoborneol/borneol is 154.25 g/mol

Mol isoborneol = 15 g/154.25 = 0.0972 mol
Mol borneol = 7.5 g/154.25 = 0.0486 mol

Use the ICE approach

        borneol  →  isoborneol
I         0.0972           0.0486
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Total moles = 0.1458

Using Raoult's Law,
Partial Pressure = Mole fraction*Total Pressure
[Partial pressure of isoborneol] = [(0.0972-x)/0.1458]*P
[Partial pressure of borneol] = [(0.0486+x/0.1458)]*P

0.106 = [(0.0972-x)/0.1458]*P/ [(0.0486+x/0.1458)]*P
Solving for x,
x = 0.0832 

Thus,
<em>Mol fraction of borneol = (0.0486+0.0832)/0.1458 = 0.904</em>
<em>Mol fraction of isoborneol = (0.0972-0.0832)/0.1458 = 0.096</em>
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